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Consider the relation,$2Ag^++Cd\rightarrow 2Ag+Cd^{+2}$ the standard electrode potentials for $Ag^+/Ag$ and $Cd^{+2}/Cd$ couples 0.8V and 0.04V respectively.What is the standard potential for this reaction?

$\begin{array}{1 1}(a)\;0.2V&(b)\;0.4V\\(c)\;0.5V&(d)\;0.3V\end{array}$

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In the given reaction $Cd$ is being oxidized to $Cd^{+2}$ ions and $Ag^+$ ions are being reduced to Ag metal.Thus the galvanic cell in which the given reaction take place can be represented as $Cd(s)/Cd^{+2}(aq)\parallel Ag^+(aq)/Ag(s)$
Thus the standard potential of given reaction would be standard emf of above cell $(E^0_{cell})$ which is given cell
$E^0_{cell}=E^0_{cathode}-E^0_{Anode}$
$\Rightarrow E^0_{Ag^+/Ag}-E^0_{Cd^{+2}/cd}$
$\Rightarrow 0.8-0.4$
$\Rightarrow 0.4V$
Hence (b) is the correct answer.
answered Feb 18, 2014 by sreemathi.v
 

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